General Chemistry: Net Ionic Equations, Neutralization Reactions, Titrations, and Redox

Vocabulary flashcards covering precipitation reactions, Brønsted-Lowry acid-base concepts, neutralization stoichiometry, titration terms, and oxidation-reduction assignment rules.

Precipitate

An insoluble solid that forms and separates out when two aqueous solutions are mixed together.

Spectator Ions

Ions that remain unchanged and dissolved in aqueous solution before and after a chemical reaction occurs.

Net Ionic Equation

A chemical equation showing only the actual reacting species involved in forming a product after canceling out spectator ions.

Brønsted-Lowry Acid

Any chemical species that acts as a proton donor, releasing $H^+$ when dissolved in $H_2O$.

Monoprotic Acid

An acid characterized by possessing and donating exactly one acidic proton.

Diprotic Acid

An acid possessing two acidic protons that it can donate, such as sulfuric acid ($H_2SO_4$).

Polyprotic Acid

An acid that contains and can donate more than two acidic protons.

Strong Electrolyte

A solute, such as a strong acid or soluble metal hydroxide base, that completely dissociates into ions in aqueous solution.

Ammonia ($NH_3$)

The single weak base introduced in the course, which reacts partially in an equilibrium reaction rather than breaking apart completely.

Salt

An ionic compound formed in a neutralization reaction, generally defined as a metal cation bonded to a nonmetal or polyatomic anion.

Neutralization Reaction

A proton transfer reaction occurring between an acid and a base that produces a salt and liquid water ($H_2O$).

Titration

An analytical laboratory technique that uses the known concentration and volume of one solution to determine the unknown concentration of another.

Indicator

A substance, such as phenolphthalein, that is colorless in acid and changes color in base to signal that moles of acid equal moles of added hydroxide.

Oxidation

A process in an electron transfer reaction characterized by the loss of electrons and an increase in oxidation number.

Reduction

A process in an electron transfer reaction characterized by the gain of electrons and a decrease in oxidation number.

Redox Reaction

An electron transfer reaction comprising simultaneous oxidation and reduction processes.

LEO the Lion Says GER

A mnemonic device representing "Lose Electrons Oxidation" ($\text{LEO}$) and "Gain Electrons Reduction" ($\text{GER}$).

Oxidation Number

A hypothetical number assigned to an element within a compound or ion to track the movement and allocation of electrons.

Rule for Free Elements

The oxidation number rule stating that any neutral, uncombined element (such as $Mg$, $Ca$, $O_2$, or $H_2$) is assigned an oxidation number of $0$.

Rule for Monatomic Ions

The oxidation number rule stating that the oxidation number of any simple monatomic ion is equal to the ionic charge on that ion.

Rule for the Sum of Oxidation Numbers

The rule stating that the sum of the oxidation numbers of all atoms in a compound or polyatomic ion must equal the overall charge on that compound or ion.

Rule for Hydrogen

The oxidation number rule stating that hydrogen is $+1$ when bonded to nonmetals and $-1$ (hydride) when bonded to metals.

Rule for Fluorine

The oxidation number rule specifying that fluorine always has an oxidation number of $-1$.

Rule for Oxygen

The oxidation number rule stating that oxygen typically has an oxidation number of $-2$ in compounds.